Matter
Substance
(Homogeneous= same throughout,
uniformly composed)
Element
-Can not be broken
down by any means
-Only ONE capital
Letter
Ex -Na
Mixtures
combined and broken down physically
Compound
-two of more
elements Combined
Chemically in a
definite ratio
- Two or more
capital letters
Ex- NaCl
Homogeneous
(same throughout)
- Solutions
- Something
dissolved into H2O
is Aqueous
Ex- NaCl(aq)= salt
water
Heterogeneous
(different
throughout)
- Garbage
-Soil
Diatomics- a group of elements that exist in pairs (theirs 7 of them!)
H2 = Hydrogen
O2= Oxygen
F2= Fluorine
Br2= Bromine
I2= Iodine
N2= Nitrogen
Cl2= Chorine
Particle Diagrams
-Monatomic elements
-Diatomic Elements
-Compound
-Mixture of elements
-Mixture of compounds
-Mixture of elements AND compounds
Formula Writing
Ionic Compounds- A transfer of electrons from a metal to a non-metal
Caton= positively charged ion (Metal of NH3)
Anion= negatively charged particle (-Non-metal or polyatomic ion Table E)
Covalent (Molecular)- a sharing of electrons between non-metals
Both qualitative and quantitative information is given in a chemical formula
Qualitative= what elements are Present
Quantitative= how many atoms of each element are present
Ex- H2OQualitative = Hydrogen, Oxygen
Quantitative = 2=Hydrogen
1= Oxygen
Counting Atoms
Coefficients represent Moles
2H2O= two moles of water
Hydrogen = 4 atoms
Oxygen = 2 atoms
If theirs Multiple polyatomic ions in a compound use parentheses
Empirical Formula
- Represents the simplest whole number ratio of atoms in a compound
-Ionic compounds are always written in empirical form
- Covalent compounds can have both a molecular form and an empirical form
- Molecular formula = represents the actual number of atoms in a molecule
Empirical
ex- C6H12O6
CH6O
Naming Covalent Compounds
Binary compound = a compound composed of two elements
All binary compounds end in the “ide” suffix
1st element =
1 atom = NO prefix
2 or more = prefix
2nd element always gets a prefix and ends in “ide”
Prefix
Mono = 1
Di = 2
Tri = 3
Tetra = 4
Penta = 5
Hexa = 6
Hepta = 7
Oct = 8
Non = 9
Deca = 10
CO2
N2O5
Carbon Dioxide
P4O10
Dinitrogen Pentoxide
Tetraphosphorus
decoxide
Naming Binary Ionic Compounds
(with 1 oxidation state)
1. CHECK for a metal
1 oxidation name the
metal as is and add “ide”
suffix to the Non-metal
2. CHECK the number of oxidation states
More than one oxidation
state use the stock system
NaCl
Sodium Chloride
AlBr3
Aluminum Bromide
Formula Writing with Binary Ionic Compounds
1. Crisscross the oxidation state to become subscripts
2. Reduce the ratio of atoms
Ex- Sodium Bromide
Na
+1
Br
Sodium Oxide
Na+1O-2
-1
NaBr
Na2O
Formula Writing- Ionic Compound containing polyatomic ions (TABLE E)
Sodium Carbonate
Aluminum Carbonate
Na+1(CO3)-2
Al+3(CO3)3
Na2CO3
Al2(CO3)3
The Stock System
The stock system is used when naming and writing formulas from a
compound in which one of the elements take on multiple oxidation states.
I = +1
II = +2
III = +3
IV = +4
V = +5
VI = +6
VII = +7
Iron (II) Oxide
Tin (II) Sulfide
Fe+2O-2
Sn+2S-2
FeO
SnS
Naming Ionic Compounds Using the Stock System
Fe2O3
Iron (III) Oxide
+6
-6
+3
Fe2
=0
-2
O3
+
1. Arrhenius acid yields an H ion as the only positive ion in the solution
therefore formulas that contain hydrogen as the first elements are acids
Binary
Table E
HF – Hydrofluoric
HCl – Hydrochloric
“Ate”  “ic”
“Ite”  “ous”
HBr – Hydrobromic
HI – Hydriodic acid
Types of Chemical Reactions
1. Synthesis = the formation of one
product
(right) from two or more reactants
(left)
2H2+O2  2H2O
2. Decomposition = the breaking down of one reactant (left) to form 2 or
more products (right)
2H2O 2H2+O2
3. Single Replacement = element1 + compound1  element2 + Compound2
In order for a single replacement reaction to occur the element must be
more active (higher on table E) then the metal in the compound
Li+NaCl Na + LiCl
4. Double Replacement = compound1 + compound2
 compound3 + compound4
NaCl + KBr  KCL + NaBr
Balancing Equations
In Chemistry there is a conservation of 3 things
1. MASS
2. CHARGE
3. ENERGY
Use coefficients (big number in front) to balance equations.
Coefficients represent the number of moles
2H2+1 O2  2H2O
When balancing equations you must use the simplest whole number
coefficients in your final answer.
2NH3 1N2+3H2
2:1:3
Sum of coefficients is 6